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NCERT Notes for Class 10, NCERT Class 10 Revision Notes - SelfStudys

After they download the well-prepared Science Class 10 Revision Notes, they can access them without worrying about the stable internet connection. The convenience of studying through professionally made notes ncdrt help students hotes excellent marks. Most importantly, students can get these Science Notes Class 10 print out in hardcopy to study at their own pace and comfort.

Chapter 1 - Chemical Reactions and Equations: Our revision notes cover all the concepts in the chapter. It offers elaborated explanations on important topics like chemical 10th Ncert English Notes Readings reactions, types ncrrt chemical reactions, how to write and balance chemical equations and. Chapter 2 - Acids, Bases, and Salts: Our 10th ncert notes 10 notes cover essential details about acids, bases, and salts, making anything taste sour or bitter.

Chapter 3 - Metals and Non-Metals: The Class 10 Science Revision Notes covers physical and chemical properties that explains the differences between metals and nonmetals. It highlights how metals and non-metals react when in contact with acids, water and metal salts. Chapter 4 ncertt Carbon and Its Compounds: Our revision notes cover all the topics mentioned in this chapter.

Students can learn about covalent compounds, four main 10tb reactions like combustion, oxidation, substitution, addition and how millions of saturated and unsaturated compounds structured in chains, rings, or branches are formed. Chapter 6 - Life Processes: Our revision Notes of Class 10 Science covers the concept of every life process, including human beings and animals.

It explains all the easy 10th ncert notes 10 that keep humans, animals, and plants alive. Chapter 7 - Control and Coordination: The crucial notes cover the concept of how living organisms owe their survival to numerous procedures, including movement and interaction.

It highlights how living organisms react to certain situations that require control and coordination. Chapter 8 - How do Organisms Reproduce: Our notes thoroughly cover the concept of reproduction in human beings, animals, and plants.

Students can understand the primary topics 10th ncert notes 10 reproduction like sexual and asexual in. Chapter 9 - Heredity and Evolution: Our Notes for Class 10 Science covers the biological inheritance, which means passing traits and features from partners to their offspring.

It also explains prime examples of evolution thoroughly. Chapter 10 - Light Reflection and Refraction: The crucial notes cover the important topic of reflection and refraction and how to calculate the nature, position, image and its magnification generated by a spherical mirror.

It 10th ncert notes 10 includes refraction of light via glass slab, the concept of refractive index and. Chapter 11 - Human Eye and Colourful World: Our notez notes cover the importance of the eye, defects of vision and their correction, atmospheric refraction, light refraction through the prism, scattering of light, Tyndall effect and. Chapter 12 - Electricity: Our notes cover all the related topics of electricity in this chapter.

Students can understand the electric current and circuit with the help of a diagram. It also includes factors on which the resistance conduct relies and the system of resistors. Chapter 13 - Magnetic Effects of Electric Current: 10th ncert notes 10 10th Science Notes cover all the significant topics like magnetic field and field lines, the force on current-carrying conductors.

It 10th ncert notes 10 covers electric motors, electric generators and domestic electric circuits in a detailed way. Chapter 14 - Sources of Energy: The crucial notes cover all 10th ncert notes 10 topics like energy, fossil fuels, conventional sources of energy and.

Students can learn alternatives or non-conventional sources of energy. Chapter 15 - Our Environment: The notes cover important aspects of our environment, ecosystem and how our activities affect the environment.

Abstract:

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Zinc does not react with cold water. Reaction of Iron with Water: Reaction of iron with cold water is very Electricity Class 10th Ncert Notes slow and comes into notice after a long time. Iron forms rust iron oxide when reacts with moisture present in the atmosphere. Iron oxide and hydrogen gas are formed by passing of steam over iron metal. Both calcium Ca and magnesium Mg are heavier than water but still float over it: Both calcium and magnesium float over water surface because hydrogen gas is evolved when these metals react with water.

It is in the form of bubbles which stick on the metal surface. Therefore, they float over it. Other metals usually do not react with water or react very slowly. Lead, copper, silver and gold do not react with steam. Reaction of metals with dilute acid: Metals form respective salts when reacting with dilute acid. Reaction of Sodium metal with dilute hydrochloric acid: Sodium metal gives sodium chloride and hydrogen gas when react with dilute hydrochloric acid.

Reaction of Magnesium metal with dilute hydrochloric acid: Magnesium chloride and hydrogen gas are formed when magnesium reacts with dilute hydrochloric acid. Reaction of Zinc with dilute sulphuric acid: Zinc sulphate and hydrogen gas are formed when zinc reacts with dilute sulphuric acid.

This method is used in the laboratory to produce hydrogen gas. Hydrogen H 2 gas is not evolved when metal is treated with nitric acid HNO 3 : Nitric acid is strong oxidising agent and it oxidises the hydrogen gas H 2 liberated into water H 2 O and itself get reduced to some oxide of nitrogen like nitrous oxide N 2 O 3 nitric oxide NO and nitrogen dioxide NO 2. Copper, gold, silver are known as noble metals. These do not react with water or dilute acids.

Metal Oxides Chemical Properties: Metal oxides are basic in nature. The aqueous solution of metal oxides turns red litmus blue. Reaction of Metal oxides with Water: Most of the metal oxides are insoluble in water. Alkali metal oxides are soluble in water. Alkali metal oxides give strong base when dissolved in water.

Reaction of Sodium oxide with Water: Sodium oxide gives sodium hydroxide when reacts with water. Reaction of Potassium oxide with Water: Potassium oxide gives potassium hydroxide when reacts with water. Reaction of Zinc oxide and Aluminium oxide: Aluminium oxide and zinc oxide are insoluble in water. Aluminium oxide and zinc oxide are amphoteric in nature. An amphoteric substance shows both acidic and basic characters.

It reacts with base like acid and reacts with an acid like a base. When zinc oxide reacts with sodium hydroxide, it behaves like an acid. In this reaction, sodium zincate and water are formed. Zinc oxide behaves like a base when reacts with acid. Zinc oxide gives zinc chloride and water on reaction with hydrochloric acid.

In a similar way, aluminium oxide behaves like a base when reacts with acid and behaves like acid when reacts with a base. Aluminium oxide gives sodium aluminate along with water when reacts with sodium hydroxide. Aluminium oxide gives aluminium chloride along with water when it reacts with hydrochloric acid. Reactivity Series of Metals: The order of intensity or reactivity of metal is known as Reactivity Series.

Reactivity of elements decreases on moving from top to bottom in the given reactivity series. In the reactivity series, copper, gold, and silver are at the bottom and hence, least reactive.

These metals are known as Noble metals. Potassium is at the top of the series and hence, most reactive.

Reaction of metals with solution of other metal salts: Reaction of metals with the solution of other metal salt is displacement reaction. In this reaction, more reactive metal displaces the less reactive metal from its salt.

Similarly, aluminium and zinc displace copper from the solution of copper sulphate. In all the above examples, iron, aluminium and zinc are more reactive than copper. This is why they displace copper from its salt solution. When copper is dipped in the solution of silver nitrate, it displaces silver and forms copper nitrate. In the reaction, copper is more reactive than silver and hence, displaces silver from silver nitrate solution.

Silver metal does not react with copper sulphate solution because silver is less reactive than copper and not able to displace copper from its salt solution. Similarly, when gold is dipped in the solution of copper nitrate, no reaction takes place because copper is more reactive than gold. In similar way, no reaction takes place when copper is dipped in the solution of aluminium nitrate because copper is less reactive than aluminium.

Non-metals are the elements that do not conduct electricity and are neither malleable nor ductile. Non-metals are the elements which form negative ions by gaining an electron.

Chemical properties of Non-metals 1. Reaction of Non-metals with Oxygen: Non-metals form respective oxide when reacting with oxygen.

When carbon is burnt in an insufficient supply of air, it forms carbon monoxide. Carbon monoxide is a toxic substance. Inhaling of carbon monoxide may prove fatal. Sulphur gives sulphur dioxide when reacting with oxygen. Sulphur catches fire when exposed to air.

When hydrogen reacts with oxygen it gives water. Non-metallic Oxide: Non-metallic oxides are acidic in nature. The solution of non-metal oxides turns blue litmus red. Carbon dioxide gives carbonic acid when dissolved in water. Sulphur dioxide gives sulphurous acid when dissolved in water. Sulphur dioxide gives sulphuric acid when reacts with oxygen. Reaction of Non-metal with Chlorine: Non-metal gives respective chloride when they react with chlorine gas.

Reaction of Non-metals with Hydrogen: Non-metals reactive with hydrogen to form covalent hydrides. Nitrogen combines with hydrogen in presence of an iron catalyst to form covalent hydride ammonia.

Reaction of Metal and Non-metal: Many metals form ionic bonds when they react with non-metals. Compounds so formed are known as Ionic Compounds. Ions: Positive or negative charged atoms are known as ions.

Ions are formed because of loss or gain of electrons. Atoms form ions obtain by the electronic configuration of the nearest noble gas. Positive ion: A positive ion is formed because of the loss of electrons by an atom. Following are some examples of positive ions: Sodium forms sodium ion because of the loss of one electron.

Because of the loss of one electron, one positive charge comes over sodium. Magnesium forms positive ion because of the loss of two electrons. Two positive charges come over magnesium because of loss of two electrons.

Negative ion: A negative ion is formed because of the gain of an electron. Some examples are given below : Chlorine gains one electron in order to achieve a stable configuration. After the loss of one electron, chlorine gets one negative charge over it forming chlorine ion.

In this course, metals get positive charge because of transfer of electrons and non-metal gets negative charge because of acceptance of electrons. In other words, bond formed between positive and negative ion is called Ionic Bond.

Since, a compound is electrically neutral, so to form an ionic compound, negative and positive both ions must be combined. Some examples are given below: Formation of Sodium Chloride NaCl : In sodium chloride, sodium is a metal alkali metal and chlorine is a non-metal.

Sodium has one valence electron and chlorine has seven valence electrons. Sodium requires losing one electron to obtain stable configuration and chlorine requires gaining one electron in order to obtain stable electronic configuration.

Thus, in order to obtain stable configuration, sodium transfers one electron to chlorine. Sodium chloride is formed because of transfer of electrons.

Thus, ionic bond is formed between sodium and chlorine. Since, sodium chloride is formed because of ionic bond, thus, it is called Ionic compound. In similar way, potassium chloride KCl is formed. Occurrence and Extraction of Metals: Minerals, ores, extraction of metals of least reactivity, extraction of metals of middle reactivity, extraction of metals of high reactivity, refining or purification of metals and corrosion.

Seawater contains many salts such as sodium chloride, magnesium chloride, etc. Mineral: Minerals are naturally occurring substances which have a uniform composition.

Ores: The minerals from which a metal can be profitably extracted are called Ores. Metals found at the bottom of reactivity series are least reactive and they are often found in nature in free-state; such as gold, silver, copper, etc. Copper and silver are also found in the form of sulphide and oxide ores.

Metals found in the middle of reactivity series, such as Zn, Fe, Pb, etc. Metals found at the top of the reactivity series are never found in free-state as they are very reactive, example; K, Na, Ca, Mg and Al, Ncert Notes For Class 10th Social Science Uk etc. Many metals are found in the form of oxides because oxygen is abundant in nature and is very reactive. Extraction of Metals: Metals can be categorised into three parts on the basis of their reactivity: Most reactive, medium reactive and least reactive.

The three major steps involved in the extraction of a metal from its ore are. Concentration of Ores: Removal of impurities, such as soil, sand, stone, silicates, etc. Ores which are mined often contain many impurities. These impurities are called gangue. First of all, concentration is done to remove impurities from ores.

The concentration of ores is also known as enrichment of ores. Process of concentration depends upon physical and chemical properties of ores. Gravity separation, electromagnetic separation, froth flotation process, etc. Conversion of Concentrated Ore into Crude Metal Conversion of metals ores into oxides: It is easy to obtain metals from their oxides. So, ores found in the form of sulphide and carbonates are first converted to their oxides by the process of roasting and calcination.

Oxides of metals so obtained are converted into metals by the process of reduction. Roasting: Heating of sulphide ores in the presence of excess air to convert them into oxides is known as Roasting.

Calcination: Heating of carbonate ores in the limited supply of air to convert them into oxides is known as Calcination. Reduction: Heating of oxides of metals to turn them into metal is known as Reduction. Cinnabar HgS is the ore of mercury. Copper glance Cu 2 S is the ore of copper. This turns HgS mercury sulphide or cinnabar into HgO mercury oxide by liberation of sulphur dioxide.

Mercury oxide so obtained is again heated strongly. This reduces mercury oxide to mercury metal. Roasting turns copper glance ore of copper into copper l oxide. Copper oxide is then heated in the absence of air. This reduces copper l oxide into copper metal. Carbonate or sulphide ores of metals 10th Ncert Notes Pdf List are first converted into respective oxides and then oxides are reduced to respective metals.

Zinc blende is roasted to be converted into zinc oxide. Zinc spar is put under calcination to be converted into zinc oxide. Zinc oxide so obtained is reduced to zinc metal by heating with carbon a reducing agent. Extraction of Iron from Haematite Fe 2 O 3 : Haematite ore is heated with carbon to be reduced to iron metal.

Extraction of Lead from Lead oxide: Lead oxide is heated with carbon to be reduced to lead metal. Reduction of Metal oxide by Heating with Aluminium: Metal oxides are heated with aluminium a reducing agent to be reduced to metal. Following is an example: Manganese dioxide and copper oxide are reduced to respective metals when heated with aluminium.

Thermite Reaction: Ferric oxide; when heated with aluminium; is reduced to iron metal. In this reaction, a lot of heat is produced.

The thermite reaction is used in the welding of electric conductors, iron joints, etc. This is also known as Thermite Welding TW. These metals cannot be reduced using carbon because carbon is less reactive than them. Electrolytic Reduction: Electric current is passed through the molten state of metal ores. Metal being positively charged is deposited over the cathode.

Example: When an electric current is passed through molten state or solution of sodium chloride, sodium metal gets deposited over the cathode. Metals obtained from the process of electrolytic reduction are pure in form. Refining or purification of metals: Metals extracted from various methods contains some impurities, thus, they are required to be refined.

Most of the metals are refined using electrolytic refining. Electrolytic Refining: In the process of electrolytic refining, a lump of impure metal and a thin strip of pure metal are dipped in the salt solution of metal to be refined. When an electric current is passed through the solution, pure metal is deposited over a thin strip of pure metal from a lump of impure metal.

In this, impure metal is used as anode and pure metal is used as a cathode. Electrolytic Refining of Copper: A lump of impure copper metal and a thin strip of pure copper are dipped in the solution of copper sulphate. Impure lump of metal is connected with the positive pole and thin strip of pure metal is connected with negative pole.

When electric current is passed through the solution, pure metal from anode moves towards cathode and is deposited over it. Impurities present in metal are settled near the bottom of anode in the solution. Settled impurities in the solution are called Anode Mud. Corrosion: Most of the metals keep on reacting with the atmospheric air.

This leads to the formation of a layer over the metal. In the long run, the underlying layer of metal keeps on getting lost due to conversion into oxides or sulphides or carbonate, etc. As a result, the metal gets eaten up. The process is called Corrosion. Rusting of Iron: Rusting of iron is the most common form of corrosion. This is the cause that long electric wires create more resistance to the electric current.

This means R will decrease with an increase in the area of conductor and vice versa. More area of conductor facilitates the flow of electric current through more area and thus, decreases the resistance. This is the cause that thick copper wire creates less resistance to the electric current. It is called the electrical resistivity of the material of conductor.

The S. Resistivity: It is defined as the resistance offered by a cube of a material of side 1m when current flows perpendicular to its opposite faces. Resistivity depends on the nature of the material of the conductor. Silver has resistivity equal to 1. Rubber and glass are very good insulators.

The resistivity of materials varies with temperature. Combination of resistors Series and Parallel combination , the heating effect of electric current and electric power. Combination of Resistors i Series combination ii Parallel combination.

Resistors in Series: When resistors are joined from end to end, it is called in series. In this case, the total resistance of the system is equal to the sum of the resistance of all the resistors in the system.

Let, three resistors R 1 , R 2 , and R 3 get connected in series. Resistors in Parallel: When resistors are joined in parallel, the reciprocal of the total resistance of the system is equal to the sum of reciprocal of the resistance of resistors.

Let three resistors R 1 , R 2 and R 3 connected in parallel. The total current through the circuit can be calculated by adding the electric current through individual resistors.

Heating Effect of Electric Current: When electric current is supplied to a purely resistive conductor, the energy of electric current is dissipated entirely in the form of heat and as a result, resistor gets heated.

The heating of resistor because of dissipation of electrical energy is commonly known as Heating Effect of Electric Current. Some examples are as follows : When electric energy is supplied to an electric bulb, the filament gets heated because of which, it gives light.

The heating of electric bulb happens because of heating effect of electric current. Cause of Heating Effect of Electric Current: Electric current generates heat to overcome the resistance offered by the conductor through which it passes.

Higher the resistance, the electric current will generate higher amount of heat. Thus, generation of heat by electric current while passing through a conductor is an inevitable consequence. This heating effect is used in many appliances, such as electric iron, electric heater, electric geyser, etc. Electric Bulb: In an electric bulb, the filament of bulb gives light because of the heating effect of electricity.

Electric Fuse: Electric fuse is used to protect the electric appliances from high voltage if any. Electric fuse is made of metal or alloy of metals, such as aluminum, copper, iron, lead, etc.

In the case of flow of higher voltage than specified, fuse wire melts and protect the electric appliances. Suppose, if an electric heater consumes W at V. Electric Power S. Unit of electric energy is kilowatt-hour kWh. Conductor: The material which can allow the flow of electrons through itself is called the conductor.

It has a large number of free electrons. It offers low opposition in the flow of current. Insulator: The material which does not allow the flow of electrons through itself is called insulator. It has less or no free electrons. It offers high opposition in the flow of current.

Electric Current: The amount of flow charge through any cross-sectional area of a conductor in unity time is called Electric Current. Electric Current is a scalar quantity.

It is measured by an ammeter. Direction: The direction of conventional current or practical current is opposite to the flow of electrons. Electric potential: Electric Potential at any point in the electric field is defined as the amount of work done to bring the unit positive charge from infinity from outside the electric field to that point. It is a scalar quantity. The -ve charge flows from lower to a higher potential.

The difference of electric potential between any two points in the electric field is called Electric Potential difference. It is known as a voltage which is equal to the work done per unit charge between two points against the static electric field.

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